Question 1

The difference in energies between the 1s and 2s orbitals is due to the penetration effect.

Accepted Answer

A) True 
 B)False  False

Question 2

Select the most basic compound from the following.

Accepted Answer

A) Bi 2O 3 
B) SiO 2 
C) Cs 2O 
D) Na 2O 
E) H 2O 
A) Bi 2O 3 
B) SiO 2 
C) Cs 2O 
D) Na 2O 
E) H 2O C

Question 3

Elements in which the outermost electron has the same principal quantum number n, show similar chemical properties.

Accepted Answer

A) True 
 B)False  False

Question 4

Select the element with the least metallic character.

Accepted Answer

A) Sn 
B) Sr 
C) Tl 
D) Ge 
E) Ga 
A) Sn 
B) Sr 
C) Tl 
D) Ge 
E) Ga

Question 5

Which of the following electron configurations is not possible for an atom in an excited state?

Accepted Answer

A) 1 s 22 s 22 p 63 s 23 p 63 d 104 s 14 p 1 
B) 1 s 22 s 22 p 63 s 13 p 5 
C) 1 s 22 s 22 p 63 s 23 p 23 d 2 
D) 1 s 22 s 22 p 63 s 23 p 63 d 104 s 2 
E) 1 s 22 s 22 p 63 s 23 p 63 d 104 s 14 p 3 
A) 1 s 22 s 22 p 63 s 23 p 63 d 104 s 14 p 1 
B) 1 s 22 s 22 p 63 s 13 p 5 
C) 1 s 22 s 22 p 63 s 23 p 23 d 2 
D) 1 s 22 s 22 p 63 s 23 p 63 d 104 s 2 
E) 1 s 22 s 22 p 63 s 23 p 63 d 104 s 14 p 3

Question 6

Select the correct set of quantum numbers (n, l, ml, ms) for the first electron removed in the formation of a cation for strontium, Sr.

Accepted Answer

A) 5, 1 , 0, −½ 
B) 5, 1, 0, ½ 
C) 5, 0, 1, ½ 
D) 5, 1, 1, ½ 
E) 5, 0, 0, −½ 
A) 5, 1 , 0, −½ 
B) 5, 1, 0, ½ 
C) 5, 0, 1, ½ 
D) 5, 1, 1, ½ 
E) 5, 0, 0, −½

Question 7

Which one of the following statements about orbital energies is incorrect?

Accepted Answer

A) In the hydrogen atom, the energy of an orbital depends only on the value of the quantum number n. 
B) In many-electron atoms the energy of an orbital depends on both n and l. 
C) Inner electrons shield outer electrons more effectively than do electrons in the same orbital. 
D) The splitting of sublevels in many-electron atoms is explained in terms of the penetration effect. 
E) The energy of a given orbital increases as the nuclear charge Z increases. 
A) In the hydrogen atom, the energy of an orbital depends only on the value of the quantum number n. 
B) In many-electron atoms the energy of an orbital depends on both n and l. 
C) Inner electrons shield outer electrons more effectively than do electrons in the same orbital. 
D) The splitting of sublevels in many-electron atoms is explained in terms of the penetration effect. 
E) The energy of a given orbital increases as the nuclear charge Z increases.

Question 8

Hund's rule is used to predict the electron configuration of atoms in excited states.

Accepted Answer

A) True 
 B)False

Question 9

When comparing the successive ionization energies of an element, an unusually big increase in ionization energy is seen when

Accepted Answer

A) the first valence electron is removed. 
B) the second valence electron is removed. 
C) the eighth electron of is removed. 
D) the first core electron is removed. 
E) the last valence electron is removed. 
A) the first valence electron is removed. 
B) the second valence electron is removed. 
C) the eighth electron of is removed. 
D) the first core electron is removed. 
E) the last valence electron is removed.

Question 10

Which of the following elements is paramagnetic?

Accepted Answer

A) Kr 
B) Zn 
C) Sr 
D) V 
E) Ar 
A) Kr 
B) Zn 
C) Sr 
D) V 
E) Ar

Question 11

Select the paramagnetic ion.

Accepted Answer

A) Cu + 
B) Ag + 
C) Fe 3+ 
D) Cd 2+ 
E) Ca 2+ 
A) Cu + 
B) Ag + 
C) Fe 3+ 
D) Cd 2+ 
E) Ca 2+

Question 12

Metallic behavior is generally associated with

Accepted Answer

A) elements with very negative electron affinities. 
B) elements with low ionization energies. 
C) elements with small atomic radii. 
D) elements with unpaired electrons. 
E) elements with partially filled p orbitals. 
A) elements with very negative electron affinities. 
B) elements with low ionization energies. 
C) elements with small atomic radii. 
D) elements with unpaired electrons. 
E) elements with partially filled p orbitals.

Question 13

Select the correct electron configuration for Te (Z = 52).

Accepted Answer

A) [Kr]5 s 25 p 64 d 8 
B) [Kr]5 s 25 d 105 p 4 
C) [Kr]5 s 24 d 105 p 6 
D) [Kr]5 s 24 f 14 
E) [Kr]5 s 24 d 105 p 4 
A) [Kr]5 s 25 p 64 d 8 
B) [Kr]5 s 25 d 105 p 4 
C) [Kr]5 s 24 d 105 p 6 
D) [Kr]5 s 24 f 14 
E) [Kr]5 s 24 d 105 p 4

Question 14

A negative electron affinity implies that the atom repels an approaching electron.

Accepted Answer

A) True 
 B)False

Question 15

Which of the following elements has the greatest atomic radius?

Accepted Answer

A) Li 
B) Ne 
C) Rb 
D) Sr 
E) Xe 
A) Li 
B) Ne 
C) Rb 
D) Sr 
E) Xe

Question 16

Energy states of atoms containing more than one electron arise from nucleus-electron and electron-electron interactions. Which of the following statements correctly describes these effects?

Accepted Answer

A) Larger nuclear charge lowers energy, more electrons in an orbital lowers energy. 
B) Larger nuclear charge lowers energy, more electrons in an orbital increases energy. 
C) Smaller nuclear charge lowers energy, more electrons in an orbital lowers energy. 
D) Smaller nuclear charge lowers energy, more electrons in an orbital increases energy. 
E) None of these choices are correct. 
A) Larger nuclear charge lowers energy, more electrons in an orbital lowers energy. 
B) Larger nuclear charge lowers energy, more electrons in an orbital increases energy. 
C) Smaller nuclear charge lowers energy, more electrons in an orbital lowers energy. 
D) Smaller nuclear charge lowers energy, more electrons in an orbital increases energy. 
E) None of these choices are correct.

Question 17

Which of the following sets of elements have the [noble gas]ns2np2 valence electron configuration?

Accepted Answer

A) O, S, Se, Te, Po 
B) N, P, As, Sb, Bi 
C) F, Cl, Br, I, At 
D) C, Si, Ge, Sn, Pb 
E) Ti, Zr, Hf 
A) O, S, Se, Te, Po 
B) N, P, As, Sb, Bi 
C) F, Cl, Br, I, At 
D) C, Si, Ge, Sn, Pb 
E) Ti, Zr, Hf

Question 18

Moseley's measurements of nuclear charges of the elements provided the basis for arranging the elements of the periodic table in order of increasing atomic number.

Accepted Answer

A) True 
 B)False

Question 19

Which of the following elements has the smallest first ionization energy?

Accepted Answer

A) Rb 
B) Mg 
C) I 
D) As 
E) F 
A) Rb 
B) Mg 
C) I 
D) As 
E) F

Question 20

In a single atom, what is the maximum number of electrons which can have quantum number n = 4?

Accepted Answer

A) 16 
B) 18 
C) 32 
D) 36 
E) None of these choices are correct. 
A) 16 
B) 18 
C) 32 
D) 36 
E) None of these choices are correct.

Exam 8: Electron Configuration and Chemical Periodicity

The difference in energies between the 1s and 2s orbitals is due to the penetration effect.

Select the most basic compound from the following.

Elements in which the outermost electron has the same principal quantum number n, show similar chemical properties.

Select the element with the least metallic character.

Which of the following electron configurations is not possible for an atom in an excited state?

Select the correct set of quantum numbers (n, l, ml, ms) for the first electron removed in the formation of a cation for strontium, Sr.

Which one of the following statements about orbital energies is incorrect?

Hund's rule is used to predict the electron configuration of atoms in excited states.

When comparing the successive ionization energies of an element, an unusually big increase in ionization energy is seen when

Which of the following elements is paramagnetic?

Select the paramagnetic ion.

Metallic behavior is generally associated with

Select the correct electron configuration for Te (Z = 52).

A negative electron affinity implies that the atom repels an approaching electron.

Which of the following elements has the greatest atomic radius?

Energy states of atoms containing more than one electron arise from nucleus-electron and electron-electron interactions. Which of the following statements correctly describes these effects?

Which of the following sets of elements have the [noble gas]ns2np2 valence electron configuration?

Moseley's measurements of nuclear charges of the elements provided the basis for arranging the elements of the periodic table in order of increasing atomic number.

Which of the following elements has the smallest first ionization energy?

In a single atom, what is the maximum number of electrons which can have quantum number n = 4?

Keys to the Study of Chemistry: Definitions, Units, and Problem Solving

The Components of Matter

Stoichiometry of Formulas and Equations

Three Major Classes of Chemical Reactions

Gases and the Kinetic-Molecular Theory

Thermochemistry: Energy Flow and Chemical Change

Quantum Theory and Atomic Structure

Models of Chemical Bonding

The Shapes of Molecules

Theories of Covalent Bonding

Intermolecular Forces: Liquids, Solids, and Phase Changes

The Properties of Mixtures: Solutions and Colloids

Periodic Patterns in the Main-Group Elements

Organic Compounds and the Atomic Properties of Carbon

Kinetics: Rates and Mechanisms of Chemical Reactions

Equilibrium: the Extent of Chemical Reactions

Acid-Base Equilibria

Ionic Equilibria in Aqueous Systems

Thermodynamics: Entropy, Free Energy, and Reaction Direction

Electrochemistry: Chemical Change and Electrical Work

The Elements in Nature and Industry

Transition Elements and Their Coordination Compounds

Nuclear Reactions and Their Applications

Filters

Select the correct set of quantum numbers (n, l, m_l, m_s) for the first electron removed in the formation of a cation for strontium, Sr.

Which of the following sets of elements have the [noble gas]ns²np² valence electron configuration?